Calcuate the tatla volme of gas (at 45c and 785mmHg) producedbby the complete decmpotition of 2.55kg of ammoniium nitrate.

To calculate the total volume of gas produced by the complete decomposition of ammonium nitrate, you need to know the balanced chemical equation for the decomposition reaction. The equation for the decomposition of ammonium nitrate is:

NH4NO3 -> N2O + 2H2O

From the equation, you can see that 1 mole of ammonium nitrate produces 1 mole of nitrogen oxide (N2O) and 2 moles of water (H2O). To find the moles of ammonium nitrate, you need to divide the mass of ammonium nitrate by its molar mass.

The molar mass of ammonium nitrate (NH4NO3) can be calculated by summing the atomic masses of each element.

NH4NO3:
(1 * atomic mass of N) + (4 * atomic mass of H) + (1 * atomic mass of O) + (3 * atomic mass of H)

Now, let's calculate the molar mass of NH4NO3:
atomic mass of N = 14.01 g/mol
atomic mass of H = 1.01 g/mol
atomic mass of O = 16.00 g/mol

Molar mass of NH4NO3 = (1 * 14.01) + (4 * 1.01) + (1 * 16.00) + (3 * 1.01) g/mol

Once you have the molar mass of NH4NO3, you can calculate the number of moles by dividing the mass of ammonium nitrate by its molar mass.

Number of moles of NH4NO3 = mass of NH4NO3 / molar mass of NH4NO3

Now that you have the number of moles of ammonium nitrate, you can determine the volume of gas produced using the ideal gas law, which states:

PV = nRT

Where:
P = pressure of the gas (785 mmHg in this case)
V = volume of the gas (what we want to calculate)
n = number of moles of gas
R = ideal gas constant (usually given as 0.0821 L·atm/(mol·K))
T = temperature of the gas (45°C converted to Kelvin)

To convert 45°C to Kelvin, you add 273.15:

T = 45 + 273.15

Now that you have the values for P, n, R, and T, you can rearrange the ideal gas law equation to solve for the volume (V):

V = (nRT) / P

Plug in the values for n, R, T, and P into the equation and calculate the volume. This will give you the total volume of gas produced by the complete decomposition of ammonium nitrate.